Question

12

1 point
The volume of a gas-filled balloon is 28 L at 40.0
°C and 222 kPa pressure. What volume will the
balloon have at 1 atm and 0 °C?
(Hint: Make sure your units are the same on both
sides of the equation)
Round to the nearest tenths place.
Type your answer...

Answer 1

To find the volume of the balloon at 1 atm and 0 °C, we can use the ideal gas law equation PV = nRT. By setting up a proportion and solving for the unknown volume, we find that the volume is approximately 0.1261 L.

Step-by-step explanation:

To solve this problem, we can use the ideal gas law equation, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.

First, we need to convert the given temperature of 40.0 °C to Kelvin by adding 273.15. This gives us a temperature of 313.15 K.

Next, we can set up a proportion using the ideal gas law equation:

1/1 = 2/2

Plugging in the given values, we get:

28 L / 222 kPa = 2 / 1 atm

Simplifying the proportion, we can cross-multiply and solve for 2:

28 * 1 = 222 * 2

2 = 28 * 1 / 222

2 ≈ 0.1261 L

Therefore, the volume of the balloon at 1 atm and 0 °C is approximately 0.1261 L.